Why decrease in the activation energy leads to  an increase in the rate of reaction?

Asked by Nishtha Sardana | 18th Jun, 2014, 04:50: PM

Expert Answer:

In the formation of product from reactant, it has to go through an intermediate stage. This stage is called transition state. The energy required for the formation of transition state from reactant is called activation energy.

If the activation energy for the reaction is lower, that causes reactant to follow a shorter path as shown in second diagram (Curve marked with pink colour). Thus, as a result the reactant has to cover a shorter distance in forming the product, it would require less time and in turn the rate of reaction will increase.

Answered by Prachi Sawant | 20th Jun, 2014, 12:24: PM